What You Should Know
So Far
The Fundamental Laws
Conservation of Mass
Definite Composition
Multiple Proportions
Daltons Atomic Theory
The Experiments
Thomson’s Cathode Ray Tube
Discovers the electron
Rutherford’s Gold Foil Experiment
Describes the atom as a small dense positively charges
nucleus surrounded by relatively large negatively
charged cloud. An atom is mostly empty space.
A wave
Amplitude
Frequency
Wavelength
What Spectrums Tell Us
Spectrum
Hydrogen Spectrum
Planks
Wave and a
Particle
Duality of Nature
Electron is both a wave and a
particle
The rules
Aufbau principle
States that the structure of each successive element is
obtained by adding one proton to the nucleus and one
electron to the lowest energy orbital that is available.
Hund’s rule
For an atom in the ground state that the number of
unpaired electrons is the maximum possible and these
unpaired electrons have the same spin
Pauli Exclusion Principle
That two particles of a certain class cannot occupy the same
four quantum numbers
Pauli’s Exclusion Principle
No two electrons can have the same four quantum numbers
orbital
Quantum Numbers
n,l,m,s
n = energy level
l = suborbital s, p,d,f
m = number of electrons
s = spin
Orbital Shapes
s orbital
p obitals
s
d orbital
f orbital
px
pz
py
Filling Electron Diagram
How To Write Configurations
Electron Arrow Diagram
Energy Level Diagram
EC Flow Chart
The Shortcut
Counting Atoms
Atomic Mass
Mass of the atom in atomic mass units
1 amu has the gram equivelence of 1 gram
Mole
SI unit for measuring the amount of substance
Carbon -12 is the standard
Exact number of atoms that is in 12.0 g of C-12
Avogadro's number
6.022 x 1023 units/mole
Mole Map
vv
HUH???
Given Moles
Given atoms
6.022 x 1023 atoms
1 mole
1 mole
6.022
x 1023 atoms
mole
==atoms
More??
Given moles
grams
Molar Weight
1 mole
Molar
1 mole
Weight
= grams
moles
LAST ONE
grams
Units
1 mole
23 units
Molar
6.022
x 10Weight
23 units
6.022
x
10
Molar Weight
1 mole
==Units
grams